{"id":143,"date":"2020-04-09T09:30:39","date_gmt":"2020-04-09T09:30:39","guid":{"rendered":"https:\/\/thechemicalelements.com\/?page_id=143"},"modified":"2023-08-15T16:43:57","modified_gmt":"2023-08-15T16:43:57","slug":"bromine","status":"publish","type":"post","link":"https:\/\/thechemicalelements.com\/bromine\/","title":{"rendered":"Bromine (Br)"},"content":{"rendered":"\n

Bromine is a nonmetallic chemical element with an atomic number of 35 in the periodic table of elements<\/a>. Its pure elemental form is rarely found in Earth\u2019s crust. Being a member of the halogen elements family<\/a> of the periodic table with seven valence electrons, bromine is highly reactive and easily makes numerous compounds with the other chemical elements.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Chemical and Physical Properties of Bromine<\/span><\/h3>\n\n\n\n
Property<\/strong><\/td>Value<\/strong><\/td><\/tr>
Symbol<\/td>Br<\/td><\/tr>
Name<\/td>Bromine<\/td><\/tr>
Atomic number<\/td>35<\/td><\/tr>
Atomic weight<\/td>79.904 g.mol-1<\/td><\/tr>
Group<\/td>Halogen<\/a><\/td><\/tr>
Period<\/td>2<\/td><\/tr>
Color<\/td>A dark reddish-brown color<\/td><\/tr>
Physical state<\/td>A fuming liquid at room temperature<\/td><\/tr>
Electronegativity<\/td>2.96<\/td><\/tr>
Density<\/td>3.119 g.cm-3 at 20\u00b0C<\/td><\/tr>
Melting point<\/td>-7.2\u00b0C<\/td><\/tr>
Boiling point<\/td>58.78\u00b0C<\/td><\/tr>
Ionic radius<\/td>1.96 (-1) \u00c5<\/td><\/tr>
Isotopes<\/td>2<\/td><\/tr>
Most characteristic isotope<\/td>Bromine-79 and bromine-81<\/td><\/tr>
Electronic shell<\/td>[Ar] 3d10 4s2 4p5<\/td><\/tr>
The energy of the first ionization<\/td>1142.7 kJ.mol-1<\/td><\/tr>
Crystal Structure<\/td>Orthorhombic<\/td><\/tr>
Shells<\/td>2,8,18,7<\/td><\/tr>
Valence<\/td>1,3,5,7<\/td><\/tr>
Covalent Radius<\/td>1.14 \u00c5<\/td><\/tr>
Atomic Radius<\/td>1.12 \u00c5<\/td><\/tr>
Atomic Volume<\/td>25.6 cm\u00b3\/mol<\/td><\/tr>
Name Origin<\/td>Greek: br\u00f4mos (stench)<\/td><\/tr>
Discoverer<\/td>Antoine J. Balard<\/td><\/tr>
Year<\/td>1826<\/td><\/tr>
Location<\/td>France<\/td><\/tr>
Pronunciation<\/td>BRO-meen<\/td><\/tr>
Oxidation States<\/td>(\u00b11),5<\/td><\/tr>
Uses<\/td>Dyes, disinfectants, photographic chemicals<\/td><\/tr>
Description<\/td>Colorless, odorless, tasteless rare noble gas<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

The reddish-brown liquid of bromine found in nature is a combination of two stable isotopes: bromine-79 (50.54 percent) and bromine-81 (49.46 percent). With the periodic table symbol Br, atomic number 35, and electron configuration [ Ar ] 3d<\/span>10<\/span> 4s<\/span>2<\/span> 4p<\/span>5<\/span>, bromine reaches its boiling point at 58.78\u00b0C, while the melting point is achieved at -7.2\u00b0C. <\/span><\/p>\n\n\n\n

Having an atomic mass of 79.904 g.mol -1, bromine is denser than water, but it\u2019s a water-soluble substance. Due to its weight, this gaseous liquid sinks in water. When the red-brown bromide gas reacts with water molecules, hydrobromic acid is produced. <\/span><\/p>\n\n\n\n

This member of the halogen family of elements in the periodic table, also labeled as Br2, has an electronegativity of 2.8 according to Pauling, whereas the atomic radius according to van der Waals is 0.165 nm. Characterized by a pungent odor, this easily evaporating gaseous substance at room temperature shares the chemical properties with chlorine<\/a> and iodine<\/a>. When compounded with phosphorus<\/a>, arsenic<\/a>, aluminium<\/a>, and antimony<\/a>, bromine forms volatile reactions. In all aggregate states, bromine retains a diatomic molecular structure.\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

How Was Bromine Discovered?<\/span><\/h2>\n\n\n\n

The Tyrian purple (the royal purple) dye was popular among the ancient civilizations. The first known chemical industry back in the times produced this ancient purple dye. It was composed of 6,6\u2032-dibromoindigo – a bromine compound. <\/span><\/p>\n\n\n\n

In 1825, the German student Carl L\u00f6wig attempted to replace chlorine with chlorine gas from a sample of magnesium<\/a> bromide-rich water from a swamp near his home in Bad Kreuznach. To conduct this experiment, the Heidelberg student used ether and the process of distillation. The result was a new chemical element – bromine. <\/span><\/p>\n\n\n\n

Upon realizing this achievement, his professor encouraged L\u00f6wig to produce more of this new chemical element. But, while he was concentrating on this feat, somewhere in France, another professor of chemistry was dedicating his time to the analysis of salt marsh waters and flora.<\/span><\/p>\n\n\n\n

Namely, a year later, in 1825, the French chemist Antoine-J\u00e9r\u00f4me Balard (1802, Montpellier, Fr. – 1876, Paris) was interested in what would result if he\u2019d distill the chlorine saturated sodium chloride and sodium sulfate crystals from seawater. <\/span><\/p>\n\n\n\n

Indeed, the liquid nonmetallic element bromine was the result of this experiment as well. Consequently, because Carl L\u00f6wig didn\u2019t publish his findings, Antoine-J\u00e9r\u00f4me Balard was recognized as the scientist who discovered the new element and its properties.\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

How Did Bromine Get Its Name?<\/span><\/h2>\n\n\n\n

As a result of its sharp and unpleasant smell, bromine was named \u201c\u03b2\u03c1\u1ff6\u03bc\u03bf\u03c2\u201d, a Greek word denoting strong stench.\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Where Can You Find Bromine?<\/span><\/h2>\n\n\n\n

Even though bromine rarely occurs in nature in its pure elemental form, traces of both soluble and insoluble bromides can be found in Earth\u2019s crust. Due to its high solubility, especially of the bromine ion (Br<\/span>\u2212<\/span>), accumulations of this nonmetallic chemical element can be found in the ocean waters. Bromine can be extracted from the ocean waters by performing chemical displacement (oxidation) with carbon tetrachloride and the addition of sulfuric acid:<\/span><\/p>\n\n\n\n

The deep ocean brine pools, natural bromide salts deposits, brines, and thermal springs are the main locations where bromine is found for commercial exploitation. In addition, the mineral bromyrite is also a source of bromine and its compounds. <\/span><\/p>\n\n\n\n

Currently, the United States, China, Mexico, Chile, Jordan, Japan, India, Ukraine, and Israel (the Dead Sea) are the world\u2019s leading bromine production countries.\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Bromine in Everyday Life<\/span><\/h2>\n\n\n\n

The two stable isotopes of bromine, bromine-79 and bromine-81, have a wide application in the medical realm, particularly in radiotherapy. Due to their sedative properties, bromides of sodium<\/a>, potassium<\/a>, calcium<\/a>, ammonium, strontium<\/a>, and lithium<\/a> were widely used at the beginning of the 20<\/span>th <\/span> century for the treatment of psychiatric patients. <\/span><\/p>\n\n\n\n

Having light-sensitive properties, silver<\/a> bromide (AgBr) is used for making photographic films, while the fire-protective materials are coated with bromine. The use as a fire retardant is also bromine\u2019s widest application in everyday life. <\/span><\/p>\n\n\n\n

Other commercial uses of bromine include water treatment, water purification, dyes, emulsion in citrus-flavored fruit drinks, as an alternative for chlorine used in swimming pools, etc.\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

How Dangerous Is Bromine?<\/span><\/h2>\n\n\n\n

Despite the fact that bromine is one of the trace elements in the human body, this chemical substance is highly toxic if inhaled. Characterized by a pungent odor, bromine is easy to detect, so any health hazards can be easily avoided. Although, man-made bromine compounds present an especially hazardous threat to human life and the environment.   <\/span><\/p>\n\n\n\n

Bromism is a syndrome that occurs as a result of bromine poisoning upon exposure to high levels of this chemical substance. This medical condition was a common occurrence due to the administration of potassium bromide, sodium bromide, and lithium bromide to psychiatric patients. These bromine-based sedatives are nowadays restricted and prohibited in many countries.  <\/span><\/p>\n\n\n\n

Bromism symptoms experienced by affected individuals include lung problems (if bromine gas is inhaled), skin irritation, coughing, burns, psychosis, fatigue, nausea, hallucinations, unresponsiveness to anything but pain, thyroid gland damage, or dysfunctionality of the nervous system. The most severe cases of bromism may have fatal effects. (<\/span>Centers for Disease Control and Prevention (CDC), National Institute for Occupational Safety and Health (NIOSH), Pocket Guide to Chemical Hazards<\/span><\/i>).<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Environmental Effects of Bromine<\/span><\/h2>\n\n\n\n

In nature, bromine occurs in many inorganic substances. As this chemical substance is often used in various industries, insecticides, and fire-extinguishers, bromide ions (Br\u2212) can additionally accumulate and contaminate water, air, and food. By releasing free bromine atoms in Earth\u2019s atmosphere, bromine has an especially negative effect on the ozone layer.\u00a0\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Isotopes of Bromine<\/span><\/h2>\n\n\n\n

Bromine has 17 radioisotopes and two stable isotopes: bromine-79 and bromine-81.<\/span><\/p>\n\n\n\n

Nuclide<\/b>\n

[n 1]<\/span><\/p>\n<\/td>

Z<\/i><\/b><\/td>N<\/i><\/b><\/td>Isotopic mass <\/b>(Da)<\/span>\n

[n 2][n 3]<\/span><\/p>\n<\/td>

Half-life<\/b><\/td>Decay<\/b>\n

mode<\/b><\/p>\n

[n 4]<\/span><\/p>\n<\/td>

Daughter<\/b>\n

isotope<\/b><\/p>\n

[n 5][n 6]<\/span><\/p>\n<\/td>

Spin and<\/b>\n

parity<\/b><\/p>\n

[n 7][n 8]<\/span><\/p>\n<\/td>

Natural abundance <\/b>(mole fraction)<\/span><\/td><\/tr>
Excitation energy<\/b><\/td>Normal proportion<\/b><\/td>Range of variation<\/b><\/td><\/tr>
68<\/span>Br<\/span>[2]<\/span><\/a><\/td>35<\/span><\/td>33<\/span><\/td>67.95836(28)#<\/span><\/td>~50 ns<\/span><\/td>p<\/span><\/td>67<\/span>Se<\/span><\/td>3+#<\/span><\/td> <\/td> <\/td><\/tr>
69<\/span>Br<\/span><\/td>35<\/span><\/td>34<\/span><\/td>68.95011(11)#<\/span><\/td><24 ns<\/span><\/td>p<\/span><\/td>68<\/span>Se<\/span><\/td>1\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
70<\/span>Br<\/span><\/td>35<\/span><\/td>35<\/span><\/td>69.94479(33)#<\/span><\/td>79.1(8) ms<\/span><\/td>\u03b2<\/span>+<\/span><\/a><\/td>70<\/span>Se<\/span><\/td>0+#<\/span><\/td> <\/td> <\/td><\/tr>
70m<\/span>Br<\/span><\/td>2292.2(8) keV<\/span><\/td>2.2(2) s<\/span><\/td>\u03b2<\/span>+<\/span><\/td>70<\/span>Se<\/span><\/td>(9+)<\/span><\/td> <\/td> <\/td><\/tr>
IT<\/span><\/a><\/td>70<\/span>Br<\/span><\/td><\/tr>
71<\/span>Br<\/span><\/td>35<\/span><\/td>36<\/span><\/td>70.93874(61)<\/span><\/td>21.4(6) s<\/span><\/td>\u03b2<\/span>+<\/span><\/td>71<\/span>Se<\/span><\/td>(5\/2)\u2212<\/span><\/td> <\/td> <\/td><\/tr>
72<\/span>Br<\/span><\/td>35<\/span><\/td>37<\/span><\/td>71.93664(6)<\/span><\/td>78.6(24) s<\/span><\/td>\u03b2<\/span>+<\/span><\/td>72<\/span>Se<\/span><\/td>1+<\/span><\/td> <\/td> <\/td><\/tr>
72m<\/span>Br<\/span><\/td>100.92(3) keV<\/span><\/td>10.6(3) s<\/span><\/td>IT (>99.9%)<\/span><\/td>72<\/span>Br<\/span><\/td>1\u2212<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>+<\/span> (<0.1%)<\/span><\/td>72<\/span>Se<\/span><\/td><\/tr>
73<\/span>Br<\/span><\/td>35<\/span><\/td>38<\/span><\/td>72.93169(5)<\/span><\/td>3.4(2) min<\/span><\/td>\u03b2<\/span>+<\/span><\/td>73<\/span>Se<\/span><\/td>1\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
74<\/span>Br<\/span><\/td>35<\/span><\/td>39<\/span><\/td>73.929891(16)<\/span><\/td>25.4(3) min<\/span><\/td>\u03b2<\/span>+<\/span><\/td>74<\/b>Se<\/b><\/td>(0\u2212)<\/span><\/td> <\/td> <\/td><\/tr>
74m<\/span>Br<\/span><\/td>13.58(21) keV<\/span><\/td>46(2) min<\/span><\/td>\u03b2<\/span>+<\/span><\/td>74<\/b>Se<\/b><\/td>4(+#)<\/span><\/td> <\/td> <\/td><\/tr>
75<\/span>Br<\/span><\/td>35<\/span><\/td>40<\/span><\/td>74.925776(15)<\/span><\/td>96.7(13) min<\/span><\/td>\u03b2<\/span>+<\/span><\/td>75<\/span>Se<\/span><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
76<\/span>Br<\/span><\/td>35<\/span><\/td>41<\/span><\/td>75.924541(10)<\/span><\/td>16.2(2) h<\/span><\/td>\u03b2<\/span>+<\/span><\/td>76<\/b>Se<\/b><\/td>1\u2212<\/span><\/td> <\/td> <\/td><\/tr>
76m<\/span>Br<\/span><\/td>102.58(3) keV<\/span><\/td>1.31(2) s<\/span><\/td>IT (99.4%)<\/span><\/td>76<\/span>Br<\/span><\/td>(4)+<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>+<\/span> (0.6%)<\/span><\/td>76<\/b>Se<\/b><\/td><\/tr>
77<\/span>Br<\/span><\/td>35<\/span><\/td>42<\/span><\/td>76.921379(3)<\/span><\/td>57.036(6) h<\/span><\/td>\u03b2<\/span>+<\/span><\/td>77<\/b>Se<\/b><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
77m<\/span>Br<\/span><\/td>105.86(8) keV<\/span><\/td>4.28(10) min<\/span><\/td>IT<\/span><\/td>77<\/span>Br<\/span><\/td>9\/2+<\/span><\/td> <\/td> <\/td><\/tr>
78<\/span>Br<\/span><\/td>35<\/span><\/td>43<\/span><\/td>77.921146(4)<\/span><\/td>6.46(4) min<\/span><\/td>\u03b2<\/span>+<\/span> (99.99%)<\/span><\/td>78<\/b>Se<\/b><\/td>1+<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span> (0.01%)<\/span><\/td>78<\/i><\/b>Kr<\/i><\/b><\/td><\/tr>
78m<\/span>Br<\/span><\/td>180.82(13) keV<\/span><\/td>119.2(10) \u00b5s<\/span><\/td> <\/td> <\/td>(4+)<\/span><\/td> <\/td> <\/td><\/tr>
79<\/span>Br<\/span><\/td>35<\/span><\/td>44<\/span><\/td>78.9183371(22)<\/span><\/td>Stable<\/b><\/td>3\/2\u2212<\/span><\/td>0.5069(7)<\/span><\/td> <\/td><\/tr>
79m<\/span>Br<\/span><\/td>207.61(9) keV<\/span><\/td>4.86(4) s<\/span><\/td>IT<\/span><\/td>79<\/b>Br<\/b><\/td>(9\/2+)<\/span><\/td> <\/td> <\/td><\/tr>
80<\/span>Br<\/span><\/td>35<\/span><\/td>45<\/span><\/td>79.9185293(22)<\/span><\/td>17.68(2) min<\/span><\/td>\u03b2<\/span>\u2212<\/span> (91.7%)<\/span><\/td>80<\/b>Kr<\/b><\/td>1+<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>+<\/span> (8.3%)<\/span><\/td>80<\/b>Se<\/b><\/td><\/tr>
80m<\/span>Br<\/span><\/td>85.843(4) keV<\/span><\/td>4.4205(8) h<\/span><\/td>IT<\/span><\/td>80<\/span>Br<\/span><\/td>5\u2212<\/span><\/td> <\/td> <\/td><\/tr>
81<\/span>Br<\/span><\/td>35<\/span><\/td>46<\/span><\/td>80.9162906(21)<\/span><\/td>Stable<\/b><\/td>3\/2\u2212<\/span><\/td>0.4931(7)<\/span><\/td> <\/td><\/tr>
81m<\/span>Br<\/span><\/td>536.20(9) keV<\/span><\/td>34.6(28) \u00b5s<\/span><\/td> <\/td> <\/td>9\/2+<\/span><\/td> <\/td> <\/td><\/tr>
82<\/span>Br<\/span><\/td>35<\/span><\/td>47<\/span><\/td>81.9168041(21)<\/span><\/td>35.282(7) h<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>82<\/b>Kr<\/b><\/td>5\u2212<\/span><\/td> <\/td> <\/td><\/tr>
82m<\/span>Br<\/span><\/td>45.9492(10) keV<\/span><\/td>6.13(5) min<\/span><\/td>IT<\/span><\/td>82<\/span>Br<\/span><\/td>2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span><\/td>82<\/b>Kr<\/b><\/td><\/tr>
83<\/span>Br<\/span><\/td>35<\/span><\/td>48<\/span><\/td>82.915180(5)<\/span><\/td>2.40(2) h<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>83<\/b>Kr<\/b><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
83m<\/span>Br<\/span><\/td>3068.8(6) keV<\/span><\/td>700(100) ns<\/span><\/td> <\/td> <\/td>(19\/2\u2212)<\/span><\/td> <\/td> <\/td><\/tr>
84<\/span>Br<\/span><\/td>35<\/span><\/td>49<\/span><\/td>83.916479(16)<\/span><\/td>31.80(8) min<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>84<\/b>Kr<\/b><\/td>2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
84m1<\/span>Br<\/span><\/td>320(10) keV<\/span><\/td>6.0(2) min<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>84<\/b>Kr<\/b><\/td>6\u2212<\/span><\/td> <\/td> <\/td><\/tr>
84m2<\/span>Br<\/span><\/td>408.2(4) keV<\/span><\/td><140 ns<\/span><\/td> <\/td> <\/td>1+<\/span><\/td> <\/td> <\/td><\/tr>
85<\/span>Br<\/span><\/td>35<\/span><\/td>50<\/span><\/td>84.915608(21)<\/span><\/td>2.90(6) min<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>85<\/span>Kr<\/span><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
86<\/span>Br<\/span><\/td>35<\/span><\/td>51<\/span><\/td>85.918798(12)<\/span><\/td>55.1(4) s<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>86<\/b>Kr<\/b><\/td>(2\u2212)<\/span><\/td> <\/td> <\/td><\/tr>
87<\/span>Br<\/span><\/td>35<\/span><\/td>52<\/span><\/td>86.920711(19)<\/span><\/td>55.65(13) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (97.48%)<\/span><\/td>87<\/span>Kr<\/span><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, <\/span>n<\/span><\/a> (2.52%)<\/span><\/td>86<\/b>Kr<\/b><\/td><\/tr>
88<\/span>Br<\/span><\/td>35<\/span><\/td>53<\/span><\/td>87.92407(4)<\/span><\/td>16.29(6) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (93.42%)<\/span><\/td>88<\/span>Kr<\/span><\/td>(2\u2212)<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (6.48%)<\/span><\/td>87<\/span>Kr<\/span><\/td><\/tr>
88m<\/span>Br<\/span><\/td>272.7(3) keV<\/span><\/td>5.4(7) \u00b5s<\/span><\/td> <\/td> <\/td> <\/td> <\/td> <\/td><\/tr>
89<\/span>Br<\/span><\/td>35<\/span><\/td>54<\/span><\/td>88.92639(6)<\/span><\/td>4.40(3) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (86.2%)<\/span><\/td>89<\/span>Kr<\/span><\/td>(3\/2\u2212,5\/2\u2212)<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (13.8%)<\/span><\/td>88<\/span>Kr<\/span><\/td><\/tr>
90<\/span>Br<\/span><\/td>35<\/span><\/td>55<\/span><\/td>89.93063(8)<\/span><\/td>1.91(1) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (74.8%)<\/span><\/td>90<\/span>Kr<\/span><\/td> <\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (25.2%)<\/span><\/td>89<\/span>Kr<\/span><\/td><\/tr>
91<\/span>Br<\/span><\/td>35<\/span><\/td>56<\/span><\/td>90.93397(8)<\/span><\/td>541(5) ms<\/span><\/td>\u03b2<\/span>\u2212<\/span> (80%)<\/span><\/td>91<\/span>Kr<\/span><\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (20%)<\/span><\/td>90<\/span>Kr<\/span><\/td><\/tr>
92<\/span>Br<\/span><\/td>35<\/span><\/td>57<\/span><\/td>91.93926(5)<\/span><\/td>0.343(15) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (66.9%)<\/span><\/td>92<\/span>Kr<\/span><\/td>(2\u2212)<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (33.1%)<\/span><\/td>91<\/span>Kr<\/span><\/td><\/tr>
93<\/span>Br<\/span><\/td>35<\/span><\/td>58<\/span><\/td>92.94305(32)#<\/span><\/td>102(10) ms<\/span><\/td>\u03b2<\/span>\u2212<\/span> (89%)<\/span><\/td>93<\/span>Kr<\/span><\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (11%)<\/span><\/td>92<\/span>Kr<\/span><\/td><\/tr>
94<\/span>Br<\/span><\/td>35<\/span><\/td>59<\/span><\/td>93.94868(43)#<\/span><\/td>70(20) ms<\/span><\/td>\u03b2<\/span>\u2212<\/span> (70%)<\/span><\/td>94<\/span>Kr<\/span><\/td> <\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (30%)<\/span><\/td>93<\/span>Kr<\/span><\/td><\/tr>
95<\/span>Br<\/span><\/td>35<\/span><\/td>60<\/span><\/td>94.95287(54)#<\/span><\/td>50# ms [>300 ns]<\/span><\/td> <\/td> <\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
96<\/span>Br<\/span><\/td>35<\/span><\/td>61<\/span><\/td>95.95853(75)#<\/span><\/td>20# ms [>300 ns]<\/span><\/td> <\/td> <\/td> <\/td> <\/td> <\/td><\/tr>
97<\/span>Br<\/span><\/td>35<\/span><\/td>62<\/span><\/td>96.96280(86)#<\/span><\/td>10# ms [>300 ns]<\/span><\/td> <\/td> <\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

Source: Wikipedia<\/span><\/p>\n\n\n\n

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List of Bromine Compounds<\/span><\/h2>\n\n\n\n

As a highly reactive septivalent chemical substance, bromine forms organo-bromides by bonding to carbon<\/a>. The most prevalent form of this carbon-bromine compound is bromomethane, also labeled as methyl bromide (CH3Br).<\/span><\/p>\n\n\n\n

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Methyl Bromide (CH<\/span>3<\/span>Br)<\/span><\/h3>\n\n\n\n

This colorless and odorless gas is considered an ozone-depleting gas when used as a fumigant. Due to this hazardous effect, it was removed from the list of allowed pesticides. In nature, bromomethane is produced by marine life and plants that belong to the cabbage and mustard family of <\/span>Brassicaceae<\/span><\/i>.\u00a0<\/span><\/p>\n\n\n\n

The list of bromine compounds comprises the following compounds with common oxidation numbers of 5, 3, 1, and -1:<\/span><\/p>\n\n\n\n